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Consider the balanced equation representing a reaction occurring in an electrolytic cell: 2NaCl → 2Na+ Cl₂ + Cl₂(8) 2(g) Where is Na produced in the electrolytic cell? A at the anode, where oxidation occurs B at the anode, where reduction occurs

Consider the balanced equation representing a reaction occurring in an electrolytic cell: 2NaCl → 2Na+ Cl₂ + Cl₂(8) 2(g) Where is Na produced in the electrolytic cell? A at the anode, where oxidation occurs B at the anode, where reduction occurs

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.65QE
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Consider the balanced equation representing a reaction occurring in an electrolytic cell:

2NaCI(l)->2Na(l)+CI2(g)

Where is Na produced in the electrolytic cell?

### Question 19 Consider the balanced equation representing a reaction occurring in an electrolytic cell: \[ 2\text{NaCl}_{(l)} \rightarrow 2\text{Na}_{(l)} + \text{Cl}_2{(g)} \] Where is Na produced in the electrolytic cell? **A.** at the anode, where oxidation occurs **B.** at the anode, where reduction occurs **C.** at the cathode, where oxidation occurs **D.** at the cathode, where reduction occurs --- In an electrolytic cell, a non-spontaneous chemical reaction is driven by an external electric current. During the electrolysis of molten sodium chloride (NaCl), sodium (Na) is produced at the cathode and chlorine gas (Cl₂) is produced at the anode. - **Cathode (site of reduction):** Sodium ions (\(\text{Na}^+\)) gain electrons (reduction) to form sodium metal (\(\text{Na}_{(l)}\)). - **Anode (site of oxidation):** Chloride ions (\(\text{Cl}^-\)) lose electrons (oxidation) to form chlorine gas (\(\text{Cl}_2{(g)}\)). Based on this understanding, the correct answer is: **D. at the cathode, where reduction occurs**
Transcribed Image Text:### Question 19 Consider the balanced equation representing a reaction occurring in an electrolytic cell: \[ 2\text{NaCl}_{(l)} \rightarrow 2\text{Na}_{(l)} + \text{Cl}_2{(g)} \] Where is Na produced in the electrolytic cell? **A.** at the anode, where oxidation occurs **B.** at the anode, where reduction occurs **C.** at the cathode, where oxidation occurs **D.** at the cathode, where reduction occurs --- In an electrolytic cell, a non-spontaneous chemical reaction is driven by an external electric current. During the electrolysis of molten sodium chloride (NaCl), sodium (Na) is produced at the cathode and chlorine gas (Cl₂) is produced at the anode. - **Cathode (site of reduction):** Sodium ions (\(\text{Na}^+\)) gain electrons (reduction) to form sodium metal (\(\text{Na}_{(l)}\)). - **Anode (site of oxidation):** Chloride ions (\(\text{Cl}^-\)) lose electrons (oxidation) to form chlorine gas (\(\text{Cl}_2{(g)}\)). Based on this understanding, the correct answer is: **D. at the cathode, where reduction occurs**
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